Does anyone have any experience with heat catalyzed crystallization of non-cannabinoid products? Like just in general?
Do you have any examples of that terminology being used in the scientific literature?
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there is such thing as inverse solubility, but that’s not what anyone’s talking about. I also suspect OP maybe isn’t using the right descriptive words to get an answer.
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Apologies definitely being a bit colloquial, but I guess I meant does any body have experience with molecules that have a S variable in the Gibbs Free Energy equation, such that an increase in temperature leads to a decrease in entropy.
Edit: what
Sulfur has a high temp (transition?) state where it gets more viscous for a short period then less.
Your body is running at 37C…does That answer your question. I think if you are looking for emergent forms in high dS/dt flow situations…you might find a “window” of
Temperature “allowance”.
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Why would that answer my question?
EDIT: ah nvm I see what you’re saying.
No it doesn’t answer my question. My question is if anyone has any experience, academic or practical, crystallizing with heat? Normally you would put a crystallization reactor at a low temperature to cause a phase change, from liquid to solid, however, there are some molecules, for instance Calcium Hydroxide, that behave in the reverse. Calcium hydroxide crystallizes under heat and is less soluble at warmer temps.
How are you making calcium hydroxide?
is it not the heating-cooling which allows a lattice to form?
Normally, I heat up my material to add to a reactor. Does that count?
Heat induced precipitation vs. supersaturation/crystallization?
Amorphous vs crystalline?
any example I could find of inverse solubility is a salt (either inorganic or a carbonate of sodium/calcium) in water. I dont think youre going to commonly find organic compounds that are inversely soluble. That said there are obviously salts of organic compounds, and perhaps those might be your best chance at finding an organic compound with inverse solubility properties.
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When labs do “jar-tek” to produce diamonds…I was under the impression the process was done at an elevated temp? I’ve always wondered about that.
[quote=“paradoxlost, post:4, topic:226694, full:true”]
Apologies definitely being a bit colloquial, but I guess I meant does any body have experience with molecules that have a S variable in the Gibbs Free Energy equation, such that an increase in temperature leads to a decrease in entropy.
Edit: on reflection I do not think I understood the exact nature of your question.
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The reason that crystalization, and many others, are performed warm/hot is for the purpose of creating crystals which exclude impurities. This is still normal solubility - impurities are more soluble in warm solution than cold.
To further demonstrate why this is not inverse solubility at play - if you rapidly cooled one of these crystallizations everything (target and impurities) could/would crash out of solution. It wouldn’t be a very selective crystallization that way.
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I have been amazed at the purity achieved by the high affinity crystallization process…a case in point, it is not even necessary to remove the 4-COOH isomer., THCA-b.
You never see it.in the COAs. I have heard of similar purities achieved with terp sauce CBDA.
When subjecting concentrated crudes obtained by base water trickery we consistently get about 90% dominant cannabinoic acid and mixture of secondary cannabinoics, in the from of off-white powders from hard vacuum rapid evaporates. (Muffins ).
I think @Alwaysworking process has to be one of the most remarkable procedures as well…If only we could get some diffraction data on those powders.
He does it completely cold…and is up there 99% purity (some sort of CRC mystery)…no chromatography .
Speaking of THCA mysteries, take a real close look at the isolation and crystallization process in Foxman’s X-ray diffraction work: (IUCr) Δ9-TetraÂhydroÂcannabinolic acid A, the precursor to Δ9-tetraÂhydroÂcannabinol (THC)
(Ref has nice 3D view of dimer centered crystal unit.)
Perhaps one needs a bit of heat to keep the side chains from freezing out “( but the conformations of the two –C5H11 chains are quite different (tgt and ttg; t is trans and g is gauche)” above ref.
I hear it’s only doing that to keep the fungi at bay…and that trick’s time is almost up, because: selection.
@paradoxlost I’m still not sure if you’re deliberately obsfucating your actual goal. Or just trying to explore the theoretical
nor that I understand the question if @eyeworm was correct here
I can wrap my head around that, and your example of Calcium Hydroxide was the only thing I found while trying to get up to speed, is there ANOTHER way to use heat to drive crystalization?
- use heat to drive evaporation; exceed solubility:crystals
- use heat to decrease (!! Fuck that’s weird!) solubility; crystallize
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Calcium Hydroxide and Calcium Sulfate seem to be the ones most commonly mentioned. I also have no clue what you’re actually getting at…
In general, crystallization is an exothermic process, while dissolution can be an endothermic or an exothermic process.
This follows Le Chatelier’s principle, but there are some exceptions…
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I’m not that was an example
I did ask a very general question, in hopes to get a very broad answer pool. I completely forgot about this equation, thank you very much. Although I don’t know if this applies that much to crystallization per say. Phase changes is definitely more a Gibbs Free Energy application because of the entropy changes. However, yes, I need to look at it from this perspective. What do you mean the “little or no temperature coefficient”? What I more mean was the S variable being such that it changes the sign in deltaH-Temperature*deltaS
You are the fucking man.
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I’m deliberately obfuscating my goal, sorry, I don’t mean to be annoying, but I’m also under an NDA.
you’re going to hate my response to the second part of your post.
evaporation prevents the crystallization of the process i’m talking about, but that has more to do with the presence of something else that if it gets too concentrated prevents crystallization.
Umm I see what you’re saying, but no this isn’t the case. Cooling causes solubility. I’m in aqueous solution btw.
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